11. Which species in the reaction below undergoes oxidation? Sn(s) 2 H (aq) a) S

Question

11. Which species in the reaction below undergoes oxidation? Sn(s) 2 H (aq) a) Sn b) Sn c) H+ d) H2 12. Determine the oxidation number of in so sulfur a) +2 b) +4 c) +6 d) +8 13. If 0.40 M of acetic acid solution has a pH of 2.57, what is the H' concentration of the solution? a) 2.7 x 103 M b) 0.039 M c) 0.40 M d) 3.7 x 102 M 14. What is the pH of a 0.34 M HNO3 solution? a) .0.47 b) 0.34 c) 0.47 d) 2.13 15. If you combine 35.0 mL of0.100 M AgNO, with 45.0 mL of 0.0800 M NaBr, what mass of AgBr is produced? a) 0.537 g b) 0.657 g c) 0.676 g d) 0.818 g Thank you. Periodic chart is attached.

Explanation / Answer

Solutions are as follows.

11. a) Sn

(goes from 0 to +2)

12. c) +6

SO4^2- : x-8 = -2; x = +6

13. a) 2.7 x 10^-3 M

pH = -log[H+] = 2.57;

14. c) 0.47

HNO3 is a strong acid, dissociates completely. Thus, [H+] concentration = 0.34 M

pH = -log(0.34) = 0.47

15. b) 0.657

1 mole of AgNO3 reacts with 1 mole of NaBr to give 1 mole of AgBr

moles of AgNO3 = M x L = 0.1 x 0.035 = 0.0035 moles

moles of NaBr = 0.08 x 0.045 = 0.0036 moles

Thus, AgNO3 is the limiting reagent in the reaction.

Moles of AgBr formed would be 0.0035 moles

Mass of AgBr produced = moles x molar mass of AgBr = 0.0036 mol x 187.77 g/mol = 0.657 g

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